It is obtained from phosphate rock or phosphorite as explained above. It exists as P₄ units where four P atoms lie at the corners of a regular tetrahedron with ∠PPP = 60^o . Each P atom is linked to three other P atoms by covalent bonds. there are total six bonds and four lone pairs of electrons present in a P₄ molecule of white phosphorus.

White phosphorus is extremely reactive due to strain in the P₄ molecule, poisonous, soft, low melting ( 317K ) solid, soluble in CS₂ , alcohols and ether. It has a garlic odour. Persons working with white P develop a disease known as Phossy jaw in which jaw bones decay. It turns yellow on exposure to light. Hence, it is also called yellow phosphorus.It spontaneously catches fire in air with a greenish glow which is visible in the dark ( P₄ + 3O₂ → P₄O₆ ) . This phenomenon is called phosphorescence. Because of its very low ignition temperature ( 303K ) , it is always kept under water.With sulfur it gives tetraphoshorus trisulphide with explosive violence which is used in “strike anywhere matches”.8P₄ + 3S₈ ——→ 8P₄S₃ With metals phosphorus forms phosphides. For example,P₄ + 6Mg ——→ 2Mg₃P₂ With aqueous alkalies, on heating, white phosphorus gives phosphine

It is an example of a disproportionation reaction where the oxidation state of P decreases from 0 to –3 (in PH₃ ) and increases to +1 (in NaH₂PO₂ )White phosphorus acts as a strong reducing agent. It reduces HNO₃ to NO₂ and H₂SO₄ to SO₂ . It also reduces solutions of Cu, Ag and Au salts to their corresponding metals. For examples,P₄ + 8CuSO₄ + 14H₂O ——→ 8Cu + 8H₂SO₄ + 4H₃PO₄

P₄ + 20AgNO₃ + 16H₂O ——→ 20Ag + 4H₃PO₄ + 20HNO₃